4. In a Daniel cell, the total reaction is given by Cu"+ZnZn2* + Cu Calculate the active mass which is necessary to deliver a capacity of 1 Ah for Zn. (atomic weight of Zn 65.4 g). Calculate the cell voltage for the Daniel cell at 298 K from AH = -210.1 kJ/mol and AS = -7.2 J/Kmol? %3D

4. In a Daniel cell, the total reaction is given by Cu"+ZnZn2* + Cu Calculate the active mass which is necessary to deliver a capacity of 1 Ah for Zn. (atomic weight of Zn 65.4 g). Calculate the cell voltage for the Daniel cell at 298 K from AH = -210.1 kJ/mol and AS = -7.2 J/Kmol? %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

4. In a Daniel cell, the total reaction is given by
Cu" + Zn - Zn2* + Cu
Calculate the active mass which is necessary to deliver a capacity of 1 Ah for Zn.
(atomic weight of Zn = 65.4 g). Calculate the cell voltage for the Daniel cell at 298 K
from AH = -210.1 kJ/mol and AS = -7.2 J/Kmol?
%3D

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